Ailine Veiga
Question: what is the heat of fusion of ice?Hypothesis: To get the heat of fusion of ice we need to determine the Energy it takes to melt the ice and also the mass of the ice and determine the heat of fusion. To determine the mass of the ice melted (m) we start by determine the volume of the water generated when the ice melted. This is the difference between the final volume (v2) and the initial volume (v1). Using the density of water (1.0g/mL), this volume can be converted into mass. This concept is shown by the equation [M= (v2-v1) x (1.0g/ml)]. To determine the energy consumed by the melting ice (E), we must determine the energy released by the water to make the ice to melt. This energy can be determined by using the equation to calculate the energy of the temperature changes. The mass of the water releasing heat is determined by multiplying the initial volume (v1) by the density of water (1.0g/mL). The specific heat of water can be obtained from any reliable reference text and is equal to 4.184j/g◦C. the temperature change is the difference between the final temperature (T2) and the initial temperature (T1) of the water. This concept is shown by the equation [E= (v1) x (1.0g/mL) x (4.184J/g°C) x (T2-T1)], and then calculate the heat of fusion of Ice using the equation EM=∆Hf. Plan: To determine the heat of fusion of ice I need a cup of warm water to place the ice cube to calculate the differences of the temperature of the warm water before the ice was add it and after the ice was added it. To take the temperature of the water we need to use a thermometer and make sure it’s in Celsius. To determine the mass, first I need to find the mass of the liquid (water) using a graduated cylinder and then find the mass again after the ice is added and then melted using the same material (graduated cylinder).

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...7/16/12
Heat of FusionHeat of Fusion for Ice
Introduction:
This lab report is a step by step process in calculating the heat of fusion for ice and to compare the differences between salt added to room temperature water and salt added to icy water. To calculate heat of fusion, one must understand heat of fusion.Heat of fusion is the amount of heat required to convert a mass of a solid at its melting point into a liquid without an increase in temperature. As difficult as this may sound, this experiment can be carried out with minimal equipment. The following equipment was needed, a 100mL graduated cylinder, a calorimeter, a digital thermometer, a calculator, water, and ice cubes.
Procedure:
The procedure to find the heat of fusion for ice was measured by melting ice cubes in a known volume and temperature of water and carefully measuring the results. The first step was to precisely measure the volume of water to be poured into the calorimeter, less then 80ml is recommended. At this point, the calorimeter water’s temperature was recorded. While continually recording the temperature, two ice cubes were dropped into the calorimeter and the temperature of the water was...

...Heat of Fusion of Ice
Experimental Data: Table 27.1
Mass of Hot Water 4.735 5.013 28.129
Hot Water Temperature 44 49 49
Final Temperature 16 23 10
Total Mass 6.097 6.138 40.830
Ice Temperature 0 0 0
Table 27.2 Calculated Data
Mass of Ice 1.362 1.125 11.674
Delta T Hot Water -28 -26 -39
Heat Lost by Water -132.6 -130.3 -1097
Delta T for Ice 16 232 10
Heat Gained by Ice 21.8 25.9 127.01
Heat Lost + Gained -110.8 -104.4 -970.0
Heat of Fusion 81.4 92.8 76.4
QUESTIONS
1. Measure the mass of the water before and after adding the ice. The difference is the mass of the ice.
2. Delta T is defined as the final temperature minus the initial temperature. The final temperature is lower than the initial temperature, so the sign is negative. The negative sign indicates the direction of the temperature change in the process. The temperature is decreased.
3. The negative sign indications the direction of energy flow; heat was lost by the water.
4. The melting point of the ice is 0. Ice and liquid water are in equilibrium at 0.
5. The positive sign means the energy flowed into the ice.
6. It’s much less than zero. The heat gained by the ice takes into account only the temperature change,...

...﻿Heat of Fusion Report Sheet
Data
Intial volume of water in the styrofoam cup (before the ice was added) (mL)
100
Final volume of water in the styrofoam cup (after the ice melted) (mL)
145
Volume of water due to melted ice (mL)
45
Mass (g) melted ice
45
Initial temperature (°C) of the water placed in the styrofoam cup
47.3
Minimum temperature (°C) after the ice was melted
45
Calculations
1. The amount of liquid water placed in the cup was _____100_______ mL. Assume that the density of water is 1.0 g/mL. What is the weight in grams of the liquid water?
Yes, because the density of water is 1
2. Calculate the temperature change.
47.3-4=43.5
3. Knowing that the specific heat of water is 4.184 J/g°C, calculate the total amount of heat released by the 100 ml of water as it cooled. This energy was used to melt the ice and then raise the temperature of the melted ice from 0 °C to the minimum temperature of the system.
Heat lost by liquid water = (mass)(specific heat)(∆T)
H=100x4.284x43.5=18200.4J
4. The amount of heat lost by the liquid water was _______18200.4j_______. Assuming that the Law of Conservation of Energy applies, the amount of heat absorbed by the melting ice was...

...Latent Heat of Fusion
Activity # 02
DE BORJA, C. A., DE CHAVES, N., DE LOS SANTOS, G. P., DEL MUNDO J., DIN, J. A., DIONISIO, J. D.
Civil Engineering Department, College of Engineering,
Adamson University
Abstract
The purpose of this experiment is to determine the Latent Heat of Fusion of ice. In this experiment, the heat of fusion of ice will be determined by using the method of mixtures
(Quantity of heat lost = Quantity of heat gained).
Introduction
When a substance changes phase, that is it goes from either a solid to a liquid or liquid to gas, the energy, it requires energy to do so. The potential energy stored in the interatomic forces between molecules needs to be overcome by the kinetic energy the motion of the particles before the substance can change phase.
The energy required to change the phase of a substance is known as a latent heat. The word latent means hidden. When the phase change is from solid to liquid we must use the latent heat of fusion, and when the phase change is from liquid to a gas, we must use the latent heat of vaporization.
Theory
When a solid has reached its melting point, additional heating melts the solid without a
temperature change. The temperature will remain constant at the melting point until the entire solid has...

...Sameera Raziuddin
Latent Heat of Fusion
April 11, 2011
Abstract: A calorimeter, water at room temperature, ice, and a Pasco GLS Explorer were used in combination with a known value of the latent heat of fusion to create and carry out an experiment to determine the mass of an unknown amount of ice. Using the formula for latent heat of fusion, the mass of theice was calculated to be 45.76g. The error of the carried out experiment was calculated to be 20.06%.
Introduction:
A substance requires energy to change from one phase state to another, or in other words, when it goes from either a solid to liquid or liquid to gas. The potential energy that is stored between molecules of the substance needs to be overcome by the kinetic energy of the motion of the particles before the substance can undergo the phase change. The temperature of a substance as heat is added to change the phase from the solid state to the gas state is shown below.
Phase changes are indicated by flat regions where heat energy is used to overcome attractive forces between molecules.
Starting a point A, the substance is in the solid state. Adding heat brings the temperature up until the substance reaches the melting point, but the material is still a solid at point B. As heat is further added,...

...Aim: Perform an experiment to determine the latent heat of fusion for milk.
Materials: Calorimeter
Celsius Thermometer
Platform balance
Kettle
Milk ice cubes
Stopwatch
Hot Water
Procedure: The copper cup was weighed and its mass was then recorded. The kettle was then used to boil water and this water was poured into the copper cup. The mass of the cup plus the hot water was calculated and recorded. The copper cup was then placed in the insulated container. The water's temperature was then recorded. The temperature of the milk ice was then recorded. The ice cub was then placed in the water. The thermometer was inserted and the temperature was taken at ten second intervals. This was done for two hundred seconds to allow the final temperature to be reached. The cup was removed from the insulated container and placed on the platform balance.
This procedure was repeated twice more to get data for a total of three trials.
Analysis: From the concept of thermal equilibrium the latent heat of fusion for milk was calculated from the data obtained from the experiment.
Q(lost) = Q(gained)
Q(gained) = Q(milk ice + milk) = mc(ice)∆T + mLf + mc(milk)∆T
Q(lost) = Q(water + cup) = m(cup)c(copper)∆T + m(water)c(water)∆T
(Working shown on following page)
From the latent heat of fusion calculated from the experiment it...

...Discussions:
1. Why theoretical value different from value obtained?
It may heat loss to the surroundings.
It may have parallax error during taking the reading.
2. Why is usually the cup used in this experiment made of polystyrene?
To prevent heat loss to the surroundings because it is a heat insulator.
3. Why the heat of neutralization has a negative sign?
The reaction gives out heat that results in the increase of temperature of the products formed.
I. Discussion
During this experiment, the pressure in the lab will be constant or essentially constant. When pressure
is constant, changes in energy (q) can be related to change in the enthalpy of reaction (ΔHrxn).
1
Energy changes accompany chemical reactions as original bonds are broken and new bonds are
formed. Usually the energy change takes the form of heat. If heat is released from the reaction, the
change in energy or enthalpy (∆H) is negative and the reaction is exothermic. Conversely, if heat is
absorbed by the reaction, the enthalpy is positive and the reaction is endothermic.
In this experiment you will measure the enthalpy (∆H) of an acid/base neutralization. A neutralization
reaction occurs when acid and base combine to form water as shown in the example below.
Overall Reaction: HCl (aq) + NaOH(aq) → NaCl(aq) + H2O(l)
TIE: H
+
(aq) + Cl
−
(aq) + Na
+
(aq) +...